Assertion: Nitrogen has higher ionization enthalpy than oxygen.
.Reason: Oxygen has stable half filled configuration .

Options

A. Assertion and reason both are correct statements and reason is correct explanation for assertion.
B. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
C. Assertion is correct statement but reason is wrong statement.
D. Assertion is wrong statement but reason is correct statement.

Answer

To analyze the given assertion and reason, we will follow these steps:

### Step 1: Understand the Assertion
The assertion states that "Nitrogen has higher ionization enthalpy than oxygen."

**Explanation**:
- Ionization enthalpy (or ionization energy) is the energy required to remove an electron from an atom in its gaseous state.
- We need to compare the ionization enthalpy of nitrogen (N) and oxygen (O).

### Step 2: Determine the Electron Configurations
- The electron configuration of nitrogen (atomic number 7) is:
- \(1s^2 2s^2 2p^3\)
- The electron configuration of oxygen (atomic number 8) is:
- \(1s^2 2s^2 2p^4\)

### Step 3: Analyze the Stability of the Electron Configurations
- Nitrogen has a half-filled p orbital configuration (2p^3), which is known to be more stable due to symmetry and exchange energy.
- Oxygen has a p orbital configuration of 2p^4, which is not half-filled.

### Step 4: Compare Ionization Energies
- Generally, atoms with half-filled or fully filled orbitals are more stable and require more energy to remove an electron.
- Therefore, nitrogen, with its half-filled p orbital, will have a higher ionization enthalpy compared to oxygen.

### Step 5: Evaluate the Reason
The reason states that "Oxygen has a stable half-filled configuration."
- This statement is incorrect because oxygen does not have a half-filled configuration; nitrogen does.

### Conclusion
- The assertion is **true**: Nitrogen has a higher ionization enthalpy than oxygen.
- The reason is **false**: Oxygen does not have a stable half-filled configuration.

### Final Answer
- Assertion: True
- Reason: False